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Electronegativity
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Electronegativity is the relative ability of an atom in a molecule to attract the electrons of a covalent bond to itself. This concept was studied by Linus Pauling, a graduate from Oregon State with a Ph.D. in chemistry. He introduced electronegativity and resonance structures. He ... was awarded the noble prize for his study of molecular structures. He discovered that the greater the electronegativity of an atom causes a stronger attraction between the electrons of the bond. The electronegativity of a atom depends on the magnitude of the core charge and on the distance the bonding pair is away from the nucleus.
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Electronegativity, EN, is an index that tells the relative attraction an element has for electrons in a bond. Electronegativity has a high value of 4.0 for F, fluorine. The lowest electronegativity value is about 0.7 for Cs, cesium. The table below shows the nonmetals have relatively high electronegativities. The metals have relatively low electronegativities. The electronegativities follow the same trends as atomic sizes (radius).
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The concept of Electronegativity refers to the ability of a bonded atom to draw electrons towards itself. It is defined as the relative ability of an atom in a molecule to attract electrons towards itself. As atoms bond, electrons are shared or transferred. The decision about sharing or transferring electrons is made based upon the electronegativities of the two bonded atoms. The atom with the higher electronegativity will dominate the electrons. The greater the difference between the electronegativity values of the two bonded atoms, the more the electrons will be transferred and the less they will be shared.
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Electronegativity is perhaps the most important periodic trend, and it is not related to ionization energy directly -- but its trend is the same, increasing from left to right. Also, the elements in a group (like the halogen group) gain stability as they grow in atomic number, so the smallest member of an electronegative group is often the most electronegative. In general, it can be said that among periods (rows) or groups (columns) of the periodic table, the closer an element is to fluorine, the more electronegative it will be. For Group VIIA (the aforementioned halogens) of the periodic table, you memorize the following relationships:
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Electronegativity is defined as the ability of an atom to withdraw electron density from a covalent bond between it and another atom. The covalent bond consists of a shared pair of electrons.
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Electronegativity